I’m very sorry but I don’t know how to answer that question.
Answer:
x-10 should be the answer
Answer:
See explanation.
Explanation:
Hello!
In this case, when having the cationic and anionic species with the specified charges, in order to abide by the net charge rule, we need to exchange the charges in the form of subscripts and without the sign, just as shown below:
Thus, for all the given combinations, we obtain:
- Y⁻

- Y²⁻

- Y³⁻

Best regards!
Both weigh in the same but the feathers has more pieces in it
Answer:a) 11.34 g of ethane
can be formed
b)
is the limiting reagent
c) 3.44 g of the excess reagent remains after the reaction is complete
Explanation:
To calculate the moles :
1. 
2. 
According to stoichiometry :
1 mole of
require 1 mole of 
Thus 0.378 moles of
will require=
of 
Thus
is the limiting reagent as it limits the formation of product and
is the excess reagent.
moles of
left = (2.10-0.378) = 1.72 moles
mass of
left=
According to stoichiometry :
As 1 mole of
give = 1 mole of 
Thus 0.378 moles of
give =
of 
Mass of 
Thus 11.34 g of ethane is formed.